(a) Following reactions occur at cathode during the electrolysis of aqueous silver chloride solution :Ag+ (aq) + e^(-) toAg (s), E° = + 0.80 V H^(+) (aq) + e^(-) to 1/2H_(2)(g) ,E^(@) = 0.00 V On the basis of their standard reduction electrode potential (E°) values, which reaction is feasible at the cathode and why? (b) Define limiting molar conductivity. Why conductivity of an electrolyte solution decreases with the decrease in concentration ?

(a) Following reactions occur at cathode during the electrolysis of aq

1.	(a) Following reactions occur at cathode during the electrolysis of aqueous silver chloride solution :Ag+ (aq) + e^(-) toAg (s), E° = + 0.80 V H^(+) (aq) + e^(-) to 1/2H_(2)(g) ,E^(@) = 0.00 V On the basis of their standard reduction electrode potential (E°) values, which reaction is feasible at the cathode and why? (b) Define limiting molar conductivity. Why conductivity of an electrolyte solution decreases with the decrease in concentration ?
Answer» Solution :(a) The reaction with a higher value of electrode potential is preferred. Hence `Ag^(+)` will be deposited in preference to `H^(+)`. `Ag^(+) (AQ) + e^(-) toAg (s) ` (b) When the concentration of the solution APPROACHES zero, molar conductivity is called limiting molar conductivity. Conductivity of an electrolyte solution decreases with decrease in concentration. Conductivity of a solution at any concentration is the conductance of one unit volume of the solution kept between platinum electrodes with unit area of cross section and at a DISTANCE of unit LENGTH. With DILUTION, the number of ions per unit volume decreases. Therefore conductivity of the solution decreases with decrease in concentration.